(a) Define the following terms :
`{:((i)"Ideal solution",(ii)"Osmitic pressure"):}`
(b) Calculate the boiling point elevation for a solution prepared by adding 10g `CaCl_(2)` to 200g of water, assuming that `CaCl_(2) `is completely dissociated.
`(K_(b)"for water"=0.512Kg mol^(-1),"Mole mass of "`CaCl_(2)=111g mol^(-1))`

Explanation

(a) (i)Ideal solution : An ideal solution of the components A and B is defined as the solution in which the intermolecular interactions between A-B are of the same magnitude as theintermolecular interactions found in the pure coponent (A-A and B-B). Example: Benzene + Toluene
(ii) Osmotic Pressure : The minimum execess pressure that has to be applied on the solution to prevent the entry of the solvent into the solution through the semipermeable membrane is called the osmotic pressure.
(b) `DeltaT_(b)=K_(b)m`
`T_(S)-T_(A)^(@)K_(b)xx(wB)/(M_(B)xxwA(kg))`
`T_(A)^(@)=100^(@)C`
`{:(w_(B)=10g,M_(B)=111g//mol),(w_(A)=10g,K_(b)=0.512kg//mol):}`
As, `CaCl toCa^(2+)+2Cl^(-)`
i = 3 [Completely dissociates]
`T_(S)-T_(A)^(@)=ixx(Kfxxw_(B))/(M_(B)xxw_(A)(kg))`
`T_(S)100=(3xx0.512xx10^(5)xx1000)/(111xx200)=0.692`
`T_(S)=100.692^(@)C`